Ch 7-10

Question 1

Principle quantum number

Answer 1

N = period of element ie row

Question 2

Angular momentum quantum number

Answer 2

l = 0,1,2,3
S,p,d,f
Shape of the orbital

Question 3

Magnetic quantum number

Answer 3

ml= 0. Only one way to orientate sphere
ml=3. -1,01
ml=5 -2,-1,0,1,2
ml=7. -3,-2,-1,0,1,2,3

Position of the orbital

Question 4

Spin quantum number

Answer 4

s=ms= -1/2 or +1/2

Question 5

Bohr atomic model

Answer 5

Electrons found in specific energy levels

Question 6

Pauli exclusion principle

Answer 6

Up spin and down spin in an orbital

Question 7

Hunds Rule

Answer 7

All up spin or all down spin filled first then opposite in orbitals

Question 8

Aufbau Principle

Answer 8

Energy orbitals fill up thru order they created by going row by row in periodic table

Question 9

Alpha decay

Answer 9

Nucleus emits an alpha particle
2 protons 2 neutrons

Question 10

Beta decay

Answer 10

Neutron turns into a proton and releases an electron

Question 11

Gamma decay

Answer 11

Nucleus at high energy
Gamma radiation released
High energy protons/neutrons drop to low energy status

Question 12

Mass defect

Answer 12

When a nucleus is split smaller pieces have larger mass than original addition

Difference in that mass is mass defect and is responsible for nuclear energy

Question 13

Nuclear fusion

Answer 13

Hydrogens make helium and mass is lost and energy is emitted

Question 14

Nuclear fission

Answer 14

Heavy atom hit by neutron therefore unstable becomes more unstable and splits

Question 15

Radioactive carbon dating

Answer 15

All organism have C14 and C12
C12 remains stable
Radioactive C14 undergo beta decay to nitrogen
C14 half-life is 5730

Question 16

Naming anions

Answer 16

Cation named first (+ charge)
Potassium ion K+

Question 17

Naming anions

Answer 17

Name element but add -ide
Cl- chloride ion

Question 18

Naming ionic compounds

Answer 18

Cation (normal) + anion (-ide)
Zinc sulfide
Potassium oxide

Question 19

Ionic transition metals - Naming

Answer 19

Iron (II) chloride

Question 20

Naming polyatomic ionic compounds

Answer 20

Cation + anion (-ate or -ite)

Question 21

NO2 -

Answer 21

Nitrite

Question 22

NO3-

Answer 22

Nitrate

Question 23

SO3-

Answer 23

Sulfite

Question 24

SO4-

Answer 24

Sulfate

Question 25

ClO-

Answer 25

Hypochlorite

Question 26

ClO2-

Answer 26

Chlorite

Question 27

ClO3-

Answer 27

Chlorate

Question 28

ClO4-

Answer 28

Perchlorate

Question 29

HCO3-

Answer 29

Hydrogen carbonate

Question 30

HSO4-

Answer 30

Hydrogen sulfate

Question 31

H2PO4

Answer 31

Dihydrogen phosphate

Question 32

KClO3

Answer 32

Potassium chlorate

Question 33

Covalent bonds properties

Answer 33

Low boiling and melting points Various colors Poor conductors of heat electricity Brittle solids Because intermolecular forces are weak

Question 34

Dipoles result in covalent bonds when

Answer 34

One atom is more electronegative than the other

Question 35

Naming covalent

Answer 35

Mono, do, tri, tetra, penta, hexa, hepta , ocata ,Nona, deca, Carbon dioxide Dinitrogen tetrachloride Phosphorus trihydride PH3

Question 36

Properties of ionic compounds

Answer 36

Form crystals High melting and boiling points Due to ionic bonds Hard and brittle Conduct electricity

Question 37

Electronegativiry

Answer 37

Ability of atom to attract shared electron pairs Smaller atoms have greater electronegativity because e- closer to nucleus

Question 38

Polar covalent bond

Answer 38

Shared electrons more atttracted to one atom with higher electronegativity

Question 39

VSEPR THEORY: valence shell electron pairs Smaller atoms repulsion theory

Answer 39

2 bonds - linear 3 bonds - trigonal planar 2 bonds - 1 e- pair = bent 4 bonds = tetrahedral 3 bonds - e- pair = trigonal pyramidal 2 bonds - 2 e- pairs = bent

Question 40

Intermolecular forces

Answer 40

Ion dipole forces Hydrogen bonding H,F, O, N Dipole dipole London dispersion forces Effect Boiling point, evaporation, solubility